2. In the previous example, you added 4 Boron-11 isotopes to 1 Boron-10 to make theaverage atomic mass 10.81.What ratio and relative percent of the isotopes were Boron-11 in the mixture?Hint: The total number of isotopes used was 5.The ratio is Boron-11 divided by Total Isotopes4124= .8 = 80%= .5 = 50%= .25 = 25%= 0.20 = 20%Submit Answer 2/2 submissions remaining

We know, average = sum of observations/ total number of observations

2. In the previous example, you added 4 Boron-11 isotopes to 1 Boron-10 to make the average atomic mass 10.81. What ratio and relative percent of the isotopes were Boron-11 in the mixture? 4)Hint: The total number of isotopes used was 5. The ratio is Boron-11 divided by Total Isotopes 4 1 2 4 = .8 = 80% = .5 = 50% = .25 = 25% = 0.20 = 20% Submit Answer 2/2 submissions remaining

2. In the previous example, you added 4 Boron-11 isotopes to 1 Boron-10 to make the average atomic mass 10.81. What ratio and relative percent of the isotopes were Boron-11 in the mixture? 4)Hint: The total number of isotopes used was 5. The ratio is Boron-11 divided by Total Isotopes 4 1 2 4 = .8 = 80% = .5 = 50% = .25 = 25% = 0.20 = 20% Submit Answer 2/2 submissions remaining

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter2: Chemical Compounds

Section: Chapter Questions

Problem 130QRT: The element bromine is Br2, so the mass of a Br2 molecule is the sum of the mass of its two atoms....

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